What mass of a non-volatile solute, urea `(NH_2CONH_2)` need to be dissolved in 100 g of water in order to decrease the vapour pressure of water by 25%? What is the molality of the solution?

The mass of a non-volatile solute of molar mass 40gmol^-1 that should be dissolved in 114 g of octane to lower its vapour pressure by 20% is

Calculate the mass of a non volatile solute (molar mass 40gmol^-1) which should be dissolved in 114 g octane to reduce its vapour pressure to 8%.

Calculate the mass of a non-volatile solute ( molar mass 40g mol^-1 ) which should be dissolved in 114g octane to reduce its vapour pressure to 80%.

2.82g of glucose are dissolved in 30g of water. Calculate the molality of the solution.

Vapour pressure of pure water at 298 k is 23.8 mm Hg. 50 g of urea (NH_2CONH_2) is dissolved in 850 g of water. Calculate the vapour pressure of water for this solution and it's relative lowering.

Find the mass of glucose that should be dissolved in 50g of water in order to produce the same lowering of vapour pressure as produce by dissolving 1 g of urea in the same quantity of water

1.0 gram of a non-volatile solute was dissolved in 100 gram of acetone (molecular mass = 58) at 298 K. The vapour pressure of solution was found to be 192.5 mm of Hg. Calculate the molecular mass of solute. The vapour pressure of pure acetone at 298 K is 195 mm of Hg.

A 3 g of urea is dissolved in 45 g of H_2O The relative lowering in Vapour pressure is